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4NH4F + 2HNO3 🔥→ 3NH4NO2 + 4HF↑ + H2↑

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Reaction of ammonium fluoride and nitric acid
4NH4FAmmonium fluoride + 2HNO3Nitric acid
🔥
⟶
3NH4NO2Ammonium nitrite + 4HF↑Hydrogen fluoride + H2↑Hydrogen

The reaction of ammonium fluoride and nitric acid yields ammonium nitrite, hydrogen fluoride, and hydrogen (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

Reaction of ammonium fluoride and nitric acid
4NH4FAmmonium fluoride + 2HNO3Nitric acid
🔥
⟶
3NH4NO2Ammonium nitrite + 4HF↑Hydrogen fluoride + H2↑Hydrogen

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of ammonium fluoride and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4FAmmonium fluoride4
Reducing
Reducing
HNO3Nitric acid2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NH4NO2Ammonium nitrite3
Redoxed product
–
HFHydrogen fluoride4
–
–
H2Hydrogen1
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of ammonium fluoride and nitric acid
4NH4FCrystalline solid + 2HNO3Liquid
🔥
⟶
3NH4NO2Crystalline solid + 4HF↑Gas + H2↑Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
350.1–––
per 1 mol of
87.53–––
per 1 mol of
175.1–––
per 1 mol of
116.7–––
per 1 mol of
87.53–––
per 1 mol of
350.1–––

Changes in aqueous solution (1)

Reaction of ammonium fluoride and nitric acid
◆
ΔrG227.3 kJ/mol
K0.15 × 10−39
pK39.82
4NH4FIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3NH4NO2Ionized aqueous solution + 4HF↑Gas + H2↑Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
479.3227.3843.8373.0
per 1 mol of
119.856.83210.993.25
per 1 mol of
239.7113.7421.9186.5
per 1 mol of
159.875.77281.3124.3
per 1 mol of
119.856.83210.993.25
per 1 mol of
479.3227.3843.8373.0

Changes in aqueous solution (2)

Reaction of ammonium fluoride and nitric acid
◆
ΔrG244.9 kJ/mol
K0.12 × 10−42
pK42.90
4NH4FIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3NH4NO2Ionized aqueous solution + 4HF↑Gas + H2↑Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
475.1244.91290–
per 1 mol of
118.861.23322.5–
per 1 mol of
237.6122.5645.0–
per 1 mol of
158.481.63430.0–
per 1 mol of
118.861.23322.5–
per 1 mol of
475.1244.91290–

Changes in aqueous solution (3)

Reaction of ammonium fluoride and nitric acid
◆
ΔrG132.8 kJ/mol
K0.54 × 10−23
pK23.27
4NH4FIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3NH4NO2Ionized aqueous solution + 4HF↑Un-ionized aqueous solution + H2↑Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
283.4132.8503.5–
per 1 mol of
70.8533.20125.9–
per 1 mol of
141.766.40251.8–
per 1 mol of
94.4744.27167.8–
per 1 mol of
70.8533.20125.9–
per 1 mol of
283.4132.8503.5–

Changes in aqueous solution (4)

Reaction of ammonium fluoride and nitric acid
◆
ΔrG150.4 kJ/mol
K0.45 × 10−26
pK26.35
4NH4FIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3NH4NO2Ionized aqueous solution + 4HF↑Un-ionized aqueous solution + H2↑Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
279.2150.4950–
per 1 mol of
69.8037.60238–
per 1 mol of
139.675.20475–
per 1 mol of
93.0750.13317–
per 1 mol of
69.8037.60238–
per 1 mol of
279.2150.4950–

Changes in aqueous solution (5)

Reaction of ammonium fluoride and nitric acid
◆
ΔrG132.8 kJ/mol
K0.54 × 10−23
pK23.27
4NH4FIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3NH4NO2Ionized aqueous solution + 4HF↑Un-ionized aqueous solution + H2↑Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
283.4132.8503.5–
per 1 mol of
70.8533.20125.9–
per 1 mol of
141.766.40251.8–
per 1 mol of
94.4744.27167.8–
per 1 mol of
70.8533.20125.9–
per 1 mol of
283.4132.8503.5–

Changes in aqueous solution (6)

Reaction of ammonium fluoride and nitric acid
◆
ΔrG150.4 kJ/mol
K0.45 × 10−26
pK26.35
4NH4FIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3NH4NO2Ionized aqueous solution + 4HF↑Un-ionized aqueous solution + H2↑Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
279.2150.4950–
per 1 mol of
69.8037.60238–
per 1 mol of
139.675.20475–
per 1 mol of
93.0750.13317–
per 1 mol of
69.8037.60238–
per 1 mol of
279.2150.4950–

Changes in aqueous solution (7)

Reaction of ammonium fluoride and nitric acid
◆
ΔrG204.9 kJ/mol
K0.13 × 10−35
pK35.90
4NH4FIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3NH4NO2Ionized aqueous solution + 4HF↑Ionized aqueous solution + H2↑Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
233.2204.993.5−170.4
per 1 mol of
58.3051.2323.4−42.60
per 1 mol of
116.6102.546.8−85.20
per 1 mol of
77.7368.3031.2−56.80
per 1 mol of
58.3051.2323.4−42.60
per 1 mol of
233.2204.993.5−170.4

Changes in aqueous solution (8)

Reaction of ammonium fluoride and nitric acid
◆
ΔrG222.5 kJ/mol
K0.10 × 10−38
pK38.98
4NH4FIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3NH4NO2Ionized aqueous solution + 4HF↑Ionized aqueous solution + H2↑Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
229.0222.5540–
per 1 mol of
57.2555.63135–
per 1 mol of
114.5111.3270–
per 1 mol of
76.3374.17180–
per 1 mol of
57.2555.63135–
per 1 mol of
229.0222.5540–

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
NH4F (cr)-463.96[1]-348.68[1]71.96[1]65.27[1]
NH4F (ai)-465.14[1]-358.09[1]99.6[1]-26.8[1]
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
NH4NO2 (cr)-256.5[1]–––
NH4NO2 (ai)-237.2[1]-111.6[1]236.4[1]-17.6[1]
HF (l)
x denotes undetermined zero point entropy
-299.78[1]–75.40+x[1]–
HF (g)-271.1[1]-273.2[1]173.779[1]29.133[1]
HF (ai)-332.63[1]-278.79[1]-13.8[1]-106.7[1]
HF (ao)-320.08[1]-296.82[1]88.7[1]–
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)